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4Cu + 2NaHSO4 🔥→ Cu2SO3 + Cu2O + Na2SO4 + H2

The reaction of copper and sodium hydrogensulfate yields copper(I) sulfite, copper(I) oxide, sodium sulfate, and hydrogen (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Reaction of oxidizable species and reducible species
Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
🔥
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper4
Reducing
Oxidizable
NaHSO4Sodium hydrogensulfate2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu2SO3Copper(I) sulfite1
Redoxed product
Cu2OCopper(I) oxide1
Oxidized
Na2SO4Sodium sulfate1
H2Hydrogen1
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of copper and sodium hydrogensulfate
ΔrG234.6 kJ/mol
K0.79 × 10−41
pK41.10
4CuCrystalline solid + 2NaHSO4Ionized aqueous solution
🔥
Cu2SO3Ionized aqueous solution + Cu2OCrystalline solid + Na2SO4Ionized aqueous solution + H2Gas
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
204.8234.6−102
per 1 mol of
51.2058.65−25.5
102.4117.3−51.0
per 1 mol of
204.8234.6−102
per 1 mol of
204.8234.6−102
per 1 mol of
204.8234.6−102
per 1 mol of
204.8234.6−102

Changes in aqueous solution (2)

Reaction of copper and sodium hydrogensulfate
ΔrG252.2 kJ/mol
K0.66 × 10−44
pK44.18
4CuCrystalline solid + 2NaHSO4Ionized aqueous solution
🔥
Cu2SO3Ionized aqueous solution + Cu2OCrystalline solid + Na2SO4Ionized aqueous solution + H2Un-ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
200.6252.2344
per 1 mol of
50.1563.0586.0
100.3126.1172
per 1 mol of
200.6252.2344
per 1 mol of
200.6252.2344
per 1 mol of
200.6252.2344
per 1 mol of
200.6252.2344

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Cu (cr)0[1]0[1]33.150[1]24.435[1]
Cu (g)338.32[1]298.58[1]166.38[1]20.786[1]
NaHSO4 (cr)-1125.5[1]-992.8[1]113.0[1]
NaHSO4 (ai)-1127.46[1]-1017.80[1]190.8[1]-38[1]
NaHSO4 (cr)
1 hydrate
-1421.7[1]-1231.6[1]155[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Cu2SO3 (ai)-492.0[1]-386.6[1]50[1]
Cu2O (cr)-168.6[1]-146.0[1]93.14[1]63.64[1]
Na2SO4 (cr)
orthorhombic
-1387.08[1]-1270.16[1]149.58[1]128.20[1]
Na2SO4 (cr)
metastable
154.934[1]129.29[1]
Na2SO4 (ai)-1389.51[1]-1268.36[1]138.1[1]-201[1]
Na2SO4 (cr)
10 hydrate
-4327.26[1]-3646.85[1]592.0[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)